Preparation of lithium carbonate from lithium chloride containing brines

ABSTRACT

This invention relates to a method for the preparation of lithium carbonate from lithium chloride containing brines. The method can include a silica removal step, capturing lithium chloride, recovering lithium chloride, supplying lithium chloride to an electrochemical cell and producing lithium hydroxide, contacting the lithium hydroxide with carbon dioxide to produce lithium carbonate.

RELATED APPLICATIONS

This application is a divisional of U.S. Ser. No. 13/617,609, filed Sep.14, 2012, which is a continuation-in-part application of U.S. Ser. No.12/766,589, filed on Apr. 23, 2010, which claims priority to U.S.Provisional Patent Application Ser. No. 61/172,540, filed on Apr. 24,2009; this application is a continuation application of U.S. Ser. No.13/612,371, filed on Sep. 12, 2012, which claims priority to U.S.Provisional Patent Application Ser. No. 61/533,561, filed on Sep. 12,2011, the disclosure of all of which are incorporated herein byreference in their entirety.

BACKGROUND OF THE INVENTION

This invention generally relates to the field of recovering lithium fromlithium containing solutions. More particularly, the invention relatesto the preparation of lithium carbonate from lithium chloride containingbrines.

DESCRIPTION OF THE PRIOR ART

It is known that geothermal brines can include various metal ions,particularly alkali and alkaline earth metals, in varyingconcentrations, depending upon the source of the brine. Recovery ofthese metals is important to the chemical and pharmaceutical industries.

Geothermal brines are of particular interest for a variety of reasons.First, geothermal brines provide a source of power due to the fact thathot geothermal pools are stored at high pressure underground, which whenreleased to atmospheric pressure, can provide a flash-steam. Theflash-stream can be used, for example, to run a power plant.Additionally, geothermal brines typically contain various useful metals,such as, lithium, lead, manganese, silver and zinc, each of which can berecovered from the brine for further use.

Lithium may be recovered from ores, as the ore may be roasted withsulfuric acid, and the product leached with water. The resulting lithiumsulfate solution is treated with lime and soda ash to remove calcium andmagnesium, and lithium is then precipitated as a carbonate. Other knownmethods for recovering lithium from ores include alkaline methods andion-exchange methods, each of which can yield solutions of lithium ashydroxide, chloride or sulfate. These methods may also include theremoval of calcium and magnesium by treatment with lime and soda ash.

Typically, the economic recovery of lithium from natural, predominantlychloride, brines (which may vary widely in composition), depends notonly on the overall lithium content, but also upon the concentrations ofinterfering ions, particularly calcium and magnesium, which can greatlyeffect the performance and economics of the lithium recovery. Magnesiumcan be difficult to remove because it is chemically similar to lithiumin solution. Generally, at low concentrations, magnesium may be removedby precipitation with lime as magnesium carbonate. At higher magnesiumconcentrations, removal with lime is not feasible and various ionexchange and liquid-liquid extraction methods have been proposed.

Although conventional processing of ores and brines makes it possible toeliminate major portions of interfering ions, there remains a need forthe simplified removal of interfering ions from brines for theproduction of lithium carbonate.

SUMMARY OF THE INVENTION

A method for the preparation of lithium carbonate from a lithiumchloride containing solution is provided. Specifically, a method for thepreparation of lithium carbonate from geothermal, smackover, and otherbrines is provided.

In one aspect, a method for preparing lithium carbonate from a lithiumchloride containing solution is provided. The method includes the stepsof supplying a lithium chloride containing solution to a silica removalstep to produce a silica-lean lithium chloride containing solution,wherein the silica removal step is operable to remove at least a portionof silica present in the lithium chloride containing stream. Thesilica-lean lithium chloride containing solution is supplied to alithium chloride capture step, wherein the lithium chloride capture stepis operable to selectively capture said lithium chloride from thesilica-lean lithium chloride containing stream. Lithium chloride isrecovered from the lithium capture step to produce a lithium chloriderich stream. The lithium chloride-rich stream is supplied to anelectrochemical cell, wherein the electrochemical cell is maintained atconditions sufficient to produce a lithium hydroxide-rich solution. Thelithium hydroxide-rich solution is contacted with carbon dioxide toproduce lithium carbonate.

In certain embodiments, the method can further include a purificationstep for decreasing the concentration of at least one of calcium,magnesium, manganese or zinc ions present in the lithium chloride richstream after the lithium chloride recovery step. The purification stepcan include the steps of contacting the lithium chloride rich streamwith a base; adding a carbonate such that at least a portion of calcium,magnesium, manganese or zinc present precipitates as a solid; andseparating the precipitate from the lithium chloride rich stream toproduce a solid waste precipitate and a purified lithium chloride richstream, said purified lithium chloride rich stream having a lowerconcentration of at least one of calcium, magnesium, manganese or zinc.

In another aspect, a method for the preparation of lithium carbonatefrom a lithium chloride containing brine solution is provided. Themethod includes the steps of providing a lithium chloride containingbrine solution. At least a portion of silica present in said lithiumchloride containing solution is removed to produce a silica-lean lithiumchloride containing solution. Lithium chloride is isolated from saidsilica-lean lithium chloride containing solution. Isolated lithiumchloride is recovered to produce a lithium chloride-rich solution. Thelithium chloride-rich solution is supplied to an electrochemical cell,which is operated at conditions sufficient to produce a lithiumhydroxide solution. Lithium hydroxide solution from said electrochemicalcell. Lithium hydroxide solution is then contacted with carbon dioxideto produce a slurry that can include lithium carbonate. Lithiumcarbonate is then recovered from the slurry.

In another embodiment, a method for preparing lithium carbonate from alithium chloride containing brine solution is provided. The method caninclude the steps of supplying a substantially silica-free lithiumchloride solution to a lithium chloride capture step, wherein thelithium chloride capture step is operable to capture a substantialportion of the lithium chloride present in the silica-lean lithiumchloride containing stream; recovering lithium chloride from the lithiumcapture step to produce a concentrated lithium chloride rich stream;contacting the concentrated lithium chloride-rich stream and a sodiumcarbonate solution in a reaction vessel, wherein said sodium carbonatesolution is prepared by contacting a sodium hydroxide solution withcarbon dioxide gas, wherein the sodium hydroxide is prepared byelectrolyzing sodium chloride; separating a product stream from thereaction vessel to provide a lithium carbonate product and a streamcomprising sodium chloride; and optionally recycling at least a portionof the sodium chloride stream to the electrochemical cell for theproduction of sodium hydroxide.

In certain embodiments, a method for preparing lithium carbonate from alithium chloride containing solution is provided. The method includesthe steps of: supplying a lithium chloride containing solution to asilica removal step to produce a silica-lean lithium chloride containingsolution; wherein the silica removal step is operable to remove at leasta portion of silica present in the lithium chloride containing stream.The method includes the step of supplying said silica-lean lithiumchloride containing solution to a lithium chloride capture step, whereinthe lithium chloride capture step is operable to capture the lithiumchloride from the silica-lean lithium chloride containing stream.Lithium chloride is recovered from the lithium capture step to produce alithium chloride rich stream. The method further includes contacting thelithium chloride rich stream with a base and adding a carbonate suchthat at least a portion of calcium, magnesium, manganese or zinc presentprecipitates as a solid. The method further includes separating theprecipitate from the lithium chloride rich stream to produce a solidwaste precipitate and a purified lithium chloride rich stream, whereinthe purified lithium chloride rich stream has a lower concentration ofat least one of calcium, magnesium, manganese or zinc. The method thenincludes the step of supplying the purified lithium chloride-rich streamto an electrochemical cell, wherein the electrochemical cell ismaintained at conditions sufficient to produce a lithium hydroxide-richsolution and contacting said lithium hydroxide-rich solution with carbondioxide to produce lithium carbonate.

In another embodiment, a method for the preparation of lithium carbonatefrom a lithium chloride containing brine solution is provided. Themethod includes the steps of: providing a lithium chloride containingbrine solution; removing at least a portion of silica present in saidlithium chloride containing solution to produce a silica-lean lithiumchloride containing solution; isolating lithium chloride from thesilica-lean lithium chloride containing solution; recovering isolatedlithium chloride to produce a lithium chloride-rich solution; contactingthe lithium chloride-rich solution with a base; adding a carbonate suchthat at least a portion of the calcium, magnesium, manganese or zincpresent precipitates as a solid; separating the precipitate from thelithium chloride rich stream to produce a solid waste precipitate and apurified lithium chloride rich stream, said purified lithium chloriderich stream having a lower concentration of at least one of calcium,magnesium, manganese or zinc; supplying the purified lithiumchloride-rich solution to an electrochemical cell and operating saidelectrochemical cell to produce a lithium hydroxide solution; recoveringthe lithium hydroxide solution from the electrochemical cell; contactingsaid lithium hydroxide solution with carbon dioxide to produce a slurrythat include lithium carbonate; and recovering lithium carbonate fromsaid slurry.

In another embodiment, a method for the preparation of lithium carbonatefrom a lithium chloride containing brine solution is provided. Themethod including the steps of supplying a substantially silica-freelithium chloride solution to a lithium chloride capture step, thelithium chloride capture step being operable to capture said lithiumchloride from the silica-lean lithium chloride containing stream. Themethod then includes the step of recovering lithium chloride from thelithium capture step to produce a concentrated lithium chloride richstream and contacting the concentrated lithium chloride rich stream witha base. A carbonate is added such that at least a portion of thecalcium, magnesium, manganese or zinc present precipitates as a solid.The method includes separating the precipitate from a purified lithiumchloride rich stream, wherein the purified lithium chloride rich streamhas a lower concentration of at least one of calcium, magnesium,manganese or zinc. The concentrated lithium chloride-rich stream and asodium carbonate solution are contacted in a reaction vessel, whereinsaid sodium carbonate solution is prepared by contacting a sodiumhydroxide solution with carbon dioxide gas, and wherein the sodiumhydroxide is prepared by electrolyzing sodium chloride. The methodfinally includes the step of separating a product stream from thereaction vessel to provide a lithium carbonate product and a streamcomprising sodium chloride.

In another embodiment, a method for the preparation of lithium carbonatefrom a lithium chloride containing brine solution is provided. Themethod includes the steps of supplying a substantially silica-freelithium chloride solution to a lithium chloride capture step, whereinthe lithium chloride capture step includes contacting the substantiallysilica-free lithium chloride solution with a lithium aluminumintercalate column that is operable to capture the lithium chloride fromthe silica-lean lithium chloride containing stream. The method includesrecovering lithium chloride from the lithium aluminum intercalate columnto produce a concentrated lithium chloride rich stream. The concentratedlithium chloride rich stream is contacted with a base. Carbonate isadded such that at least a portion of the calcium, magnesium, manganeseor zinc present precipitates as a solid. The method includes separatingthe precipitate from a purified lithium chloride rich stream, whereinthe purified lithium chloride rich stream has a lower concentration ofat least one of calcium, magnesium, manganese or zinc. The method thenincludes the step of contacting the purified lithium chloride-richstream and a sodium hydroxide solution in a reaction vessel to produce asolution comprising lithium hydroxide, wherein the sodium hydroxidesolution can be prepared by electrolyzing sodium chloride in anelectrochemical cell. The electrochemical cell can include an anode, acathode, and a semi-permeable membrane separating an anode chamber and acathode chamber. The method includes the step of contacting the solutionthat includes lithium hydroxide with carbon dioxide gas in a reactionvessel to produce a solution that includes lithium carbonate; andseparating a product stream from the reaction vessel to provide alithium carbonate product and a stream comprising sodium chloride.

In another embodiment, a method for purifying a lithium chloridecontaining solution is provided. The method includes the steps of:providing a lithium chloride containing feed solution and contacting thelithium chloride containing feed solution with a solvent extractionmixture. The solvent extraction mixture being operable to remove atleast a portion of the divalent ions present in the lithium chloridecontaining feed solution. The method then includes the step of producinga purified lithium chloride containing solution having a reducedconcentration of divalent ions relative to the lithium chloridecontaining feed solution.

In certain embodiments, the solvent extraction mixture comprisesphosphinic acid. In alternate embodiments, the extraction mixturecomprises petroleum distillates. In other embodiments, the solventextraction mixture comprises a mixture of phosphinic acid and petroleumdistillates. In certain embodiments, the method further includes stepsfor preparing lithium carbonate from a lithium chloride-rich stream. Themethod includes the steps of: converting the lithium chloride in thepurified lithium chloride-rich stream to lithium carbonate. Theconversion step can include supplying the purified lithium chloride-richstream to an electrochemical cell, wherein the electrochemical cell ismaintained at conditions sufficient to produce a lithium hydroxide-richsolution; and contacting said lithium hydroxide-rich solution withcarbon dioxide to produce lithium carbonate.

In certain embodiments, the method includes steps for the removal ofsilica prior to the extraction step. The steps include supplying thegeothermal brine to a silica removal step to produce a silica-leanlithium chloride containing solution relative to the geothermal brine;said silica removal step operable to remove at least a portion of silicapresent in the geothermal brine. The method can also include steps forconcentrating the lithium chloride prior to the extraction step, whichincludes supplying said silica-lean lithium chloride containing solutionto a lithium chloride capture step, said lithium chloride capture stepbeing operable to capture said lithium chloride from the silica-leanlithium chloride containing stream.

The method can also include steps for preparing lithium hydroxide from alithium chloride-rich stream. The lithium hydroxide preparationincluding the steps of converting the lithium chloride in the purifiedlithium chloride-rich stream to lithium hydroxide. The conversion caninclude contacting the purified lithium chloride-rich stream and asodium hydroxide solution in a reaction vessel to produce a solutioncomprising lithium hydroxide, wherein said sodium hydroxide solution isprepared by electrolyzing sodium chloride in an electrochemical cell,said electrochemical cell comprising an anode, a cathode, and asemi-permeable membrane separating an anode chamber and a cathodechamber.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1 is a flow chart of the steps of a method for the production oflithium hydroxide from a geothermal brine according to one embodiment.

FIG. 2 is a flow chart of the steps of a method for the production oflithium carbonate from a geothermal brine according to one embodiment.

FIG. 3 is a schematic diagram of one embodiment of an apparatus for theproduction of lithium carbonate from a geothermal brine according to oneembodiment.

FIG. 4 is a schematic diagram of one embodiment of an apparatus for theproduction of lithium carbonate from a geothermal brine according to oneembodiment.

FIG. 5 is a schematic diagram of one embodiment of an apparatus for theproduction of lithium carbonate from a geothermal brine according to oneembodiment.

FIG. 6 shows the compares of lithium hydroxide concentration formultiple embodiments.

FIG. 7 shows variation of cell voltage of an electrolysis cell duringpreparation of lithium hydroxide in one embodiment.

FIG. 8 shows lithium hydroxide concentration as a function of currentefficiency in one embodiment.

FIG. 9 shows energy consumption for production of lithium hydroxide inone embodiment.

FIG. 10 is a schematic diagram of one embodiment of an apparatus for theproduction of lithium carbonate from a geothermal brine according to oneembodiment.

FIG. 11 is a schematic diagram of an embodiment for concentrating theconcentration of lithium chloride in a lithium chloride containingstream.

FIG. 12 is a schematic diagram of an embodiment for concentrating alithium chloride stream.

DETAILED DESCRIPTION OF THE INVENTION

Broadly, described herein are methods for the production of lithiumhydroxide and lithium carbonate from a lithium chloride containingsolution.

As shown in FIG. 1, in one embodiment, the method generally includes astep of providing a lithium chloride containing solution, such as forexample, a geothermal brine, a silica removal step, a lithium chlorideextraction step, an optional lithium chloride concentration step, anelectrochemical lithium hydroxide production step, an evaporation step,and a lithium hydroxide isolation and drying step.

As shown in FIG. 2, in one embodiment, the method generally includes astep of providing a lithium chloride containing solution, such as forexample, a geothermal brine, a silica removal step, a lithium chlorideextraction step, an optional lithium chloride concentration step, anelectrochemical lithium hydroxide production step, and a carbonationstep, whereby lithium hydroxide is converted to lithium carbonate.

As used herein, brine solution refers to a solution of alkali and/oralkaline earth metal salt(s) in water, wherein the concentration ofsalts can vary from trace amounts up to the point of saturation.Generally, brines suitable for the methods described herein can beaqueous solutions that may include alkali metal or alkaline earthchlorides, bromides, sulfates, hydroxides, nitrates, and the like, aswell as natural brines. Brines can be obtained from natural sources,such as, Chilean brines or Salton Sea geothermal resource brines,geothermal brines, sea water, mineral brines (e.g., lithium chloride orpotassium chloride brines), alkali metal salt brines, and industrialbrines, for example, industrial brines recovered from ore leaching,mineral dressing, and the like. The present methods are equallyapplicable to artificially prepared lithium chloride solutions.

Accordingly, the present methods include the preparation and recovery oflithium carbonate from solutions that include monovalent cations,including lithium, multivalent cations, monovalent anions, andmultivalent anions.

In certain embodiments, silica may be present in the lithium chloridecontaining solution or geothermal brine, and may be removed by a varietyof known methods (e.g., U.S. Pat. No. 4,016,075), prior to use in themethods described herein. Thus, in certain embodiments, the methods forthe preparation of lithium carbonate described herein can include asilica management step.

Referring to FIG. 1, provided herein is a multistep method for theisolation of lithium ions from a brine or other lithium containingsolution and the subsequent production of lithium carbonate therefrom.In a first step of the method, the brine is supplied to a silicamanagement step, wherein silica is removed from the brine to produce asilica-free brine or lithium containing solution. In a second step ofthe method, lithium ions are removed from the silica-free brine orlithium containing solution. Optionally, in a third step, the lithiumion containing solution from the second step may be concentrated toproduce a concentrated lithium ion containing solution. In a fourthstep, the lithium containing solution is supplied to an electrochemicalcell to produce a lithium hydroxide containing solution. In a fifthstep, water can be removed from the lithium hydroxide containingsolution from step 4 to crystallize at least a portion of the lithiumhydroxide from step 4. In a sixth step, the lithium hydroxide isisolated, recovered, and dried.

Referring to FIG. 2, provided is a multistep method for the isolation oflithium ions from a brine or other lithium containing solution and thesubsequent production of lithium carbonate therefrom. In a first step ofthe method, a brine is supplied to a silica management step, whereinsilica is removed from the brine to produce a silica-free brine orlithium containing solution. In a second step, lithium ions are removedfrom the silica-free brine or lithium containing solution. In anoptional third step, the lithium ion containing solution can beconcentrated to produce a concentrated lithium ion containing solution.In a fourth step, the lithium containing solution is supplied to anelectrochemical cell to produce lithium hydroxide. The lithium hydroxidecan be supplied to a fifth step where lithium hydroxide is converted tolithium carbonate. In a sixth step, lithium carbonate is isolated andrecovered.

Referring to FIG. 3, in one embodiment of the present method, lithiumchloride containing solution 10 is provided. As noted above, lithiumchloride containing solution 10 can be obtained from a variety ofsources, including geothermal brines. The lithium chloride containingsolution is supplied to silica management step 12, which operates tosignificantly reduce the amount of silica that may be present in lithiumchloride containing solution 10, such that silicate precipitate 16 andsilica-lean lithium chloride containing solution 14 are produced.Preferably, after the silica management step, the silicon concentrationin silica-lean lithium chloride containing solution 14 is less thanabout 150 ppm, more preferably the concentration is less than about 100ppm, even more preferably the concentration is less than about 50 ppm,and even more preferably the concentration is less than about 25 ppm. Incertain embodiments, the concentration of silicon in silica-lean lithiumchloride containing solution 14 is less than about 20 ppm, less thanabout 10 ppm, or even less than about 5 ppm. It is understood that thesilica management step may be omitted from the process for brines thatdo not include silica, or brines that have a substantially low initialsilica concentration.

In certain embodiments, silica management step 12 can include the stepof contacting lithium chloride containing solution 10 with activatedalumina to remove at least a portion of the silica present. Alumina thatincludes silica bound thereto can be regenerated by contacting thealumina with sodium hydroxide. Alternatively, the lithium chloridecontaining solution can be contacted with aluminum chloride, which isconverted to aluminum hydroxide, and can be used to precipitate silicapresent in the lithium chloride containing stream. In a furtherembodiment, iron (II) that may be present in certain lithium containingbrines can be oxidized with an oxidant, such as air, hypochlorite,hydrogen peroxide, oxygen, ozone, or a like oxidizing agent, to generateiron (III) chloride, which after adjustment of the pH to above about 5,from an initial pH of about 2.5 to 3.5, will precipitate ferrichydroxide. The ferric hydroxide can adsorb silica from the lithiumcontaining brine. In a preferred embodiment, the pH is adjusted tobetween about 5 and 6 to induce precipitation of silica and iron. Inalternate embodiments, the pH is adjusted to above at least about 4.5 toinduce precipitation of silica and iron. In certain embodiments, it ispreferred the pH is not increased above about 6, to prevent theprecipitation of other ionic species present in the lithium containingbrine. In yet another embodiment, iron (II) can be added to the lithiumchloride containing solution and oxidized by known means to iron (III),such as with by contacting the iron (II) with an oxidant, such as air,oxygen, ozone, hypochlorite, hydrogen peroxide, or other suitableoxidizing agent. Contacting silica present in the lithium chloridecontaining solution with the iron (III) compound forms a precipitatewhen the pH is adjusted to between about 4.5 and 6 with the addition oflime or similar base. It a preferred embodiment, the pH is adjusted tobetween about between about 5 and 6. In alternate embodiments, the pHmust be adjusted to above at least about 4.5 for the silica and iron toprecipitate. In certain embodiments, it is preferred the pH is notincreased above about 6, to prevent the precipitation of other ionicspecies.

In addition, silica management step 12 can include any known means forremoving a portion of the silica present in the feed stream, while atthe same time maintaining the initial concentration of lithium. In oneembodiment, lithium chloride containing solution 10 can be contactedwith aluminum chloride, iron chloride, aluminum hydroxide, or the like,to form a precipitate with the silica. Contacting can be facilitated byknown means, such as a mixing device. Solid silica precipitate 16removed from lithium chloride containing solution 10 can be collectedand removed from the mixing or like device, by known means, such asscreening or filtering, to yield lithium chloride containing stream 14that is substantially free of silica.

As known in the art, various membranes can be used to selectively removespecific undesired ions from lithium containing solution 14.

Silica-lean lithium chloride containing stream 14, which issubstantially free of silica (measured as SiO₂), can be supplied tolithium chloride isolation step. In certain embodiments, silica-leanlithium chloride containing stream 14 can be supplied to at least oneintercalated lithium absorbent column 18, which can be configured toabsorb and isolate lithium chloride from the silica-lean lithiumchloride containing solution, while at the same time allowing otherions, such as calcium, magnesium, and/or sodium, or the like, to passwith water stream 22, through the use of a selective molecular sieve,membrane, or other like materials. In embodiments that include more thanone intercalated lithium absorbent column, the bulk of the lithium canbe removed in the first intercalated lithium absorbent column, with anysubsequent “polishing” intercalated lithium absorbent columns being usedto minimize overall lithium loss during the recovery process.

In certain embodiments, the intercalated lithium absorbent column can beoperated as follows. Lithium alumina intercalate particles having anaverage diameter of between about 100 and 150 μm can be combined with asaturated sodium chloride solution that includes approximately 200 ppmlithium chloride to prepare a slurry, which can then be added to thecolumn. The column may be jacketed, insulated or may include means toprovide heating or cooling to the column. The column may include amethod of distributing liquid and support for the extraction media andcan include fitted ends having a pore size of between approximately 25and 50 μm, although other like means, such as supports of glass wool orperforated plates, can also be used instead of fritted ends. Suchdesigns also include fractals. For the present invention, the operatingtemperature of the column can be maintained at a temperature that isgreater than room temperature, and is preferably maintained at atemperature above about 70° C., more preferably between about 95° C. and110° C.

The column is maintained wet and is unloaded before the first use bycirculating at least about 1 bed volume, preferably about two bedvolumes, of deionized water 20 that includes approximately 1000 ppmlithium chloride, at a flow rate of between approximately 1 and 4 bedvolumes/hour, preferably between about 1.5 and 2.5 bed volumes/hour. Thecolumn is then contacted with approximately one bed volumes of saturatedsodium chloride solution containing approximately 500 ppm lithiumchloride is then run.

During loading of the column (i.e., during the step of capturing desiredlithium chloride), high ionic strength solution 14 containing lithiumchloride is supplied to column 18 and the lithium concentration of theeffluent at column outlet 22 is measured to determine the point at whichthe column becomes saturated with the lithium chloride. During thelithium ion capture step, the lithium concentration at outlet 22 remainsfairly constant and relatively low, for example, approximately 0 and 100ppm. The point at which column 18 reaches or nears the point ofsaturation with lithium ions, however, the concentration of the lithiumin the effluent increases, thus indicating that the column has eitherlittle or no capacity for additional lithium ions. Upon reaching thispoint of saturation, flow of the solution that includes lithium chlorideto column 18 stopped, and the column is flushed with between about 1 and8 bed volumes of deionized water, preferably between about 1 and 2.5 bedvolumes, and most preferably between about 1 and 1.5 bed volumes, toproduce a lithium chloride-rich stream 24. It is understood that theapparatus can include various valves and control devices for controllingthe flow of the lithium containing solution or the wash solution to thecolumn.

In certain embodiments, after loading of the column, but beforecollection of the captured lithium chloride, the column may be flushedwith about 1 bed volume of a 26% saturated sodium chloride solution thatincludes about 200 ppm lithium chloride.

After the removal of lithium chloride from the lithium containing feedstream during the lithium chloride isolation step, intercalated lithiumabsorbent columns 18 can be regenerated and the lithium chloriderecovered therefrom. Specifically, at least about 0.5 equivalents ofwash water 20 may be supplied to column(s) 18 to remove absorbed lithiumchloride and produce lithium chloride rich solution 24. In certainembodiments, between about 1 to 2 equivalents of wash water 20, or moreequivalents, may be used during the regeneration of the columns. Inpreferred embodiments, the wash water may include lithium ions for theregeneration of the columns. Optionally, low ionic strength liquids,such as alcohols and water/alcohol mixtures can be used to regeneratethe columns. In general, the amount of water utilized from the lithiumchloride recovery from the column is minimized by recycling the productstreams to maximize lithium content, without affecting the capacity ofthe extracting media.

Optionally, a purification step can be employed to remove calcium,magnesium, or other divalent ions such as zinc and manganese that may bepresent in lithium chloride-rich stream 24. Removal of calcium,magnesium, and/or other alkaline earth metals can be achieved by knownmeans, such as, by increasing the pH and treating the solution with ionexchange, preferably using selective chelating ion exchange resins, orby the addition of a base, such as lime, sodium hydroxide, lithiumhydroxide, or the like, followed by the addition of lithium carbonate,sodium carbonate, potassium carbonate, ammonium carbonate, or othersuitable carbonate, which can precipitate magnesium and iron hydroxide,as well as calcium carbonate. In alternate embodiments, ion exchangemeans can be employed to facilitate the removal of calcium, magnesium,and/or other alkaline earth metals. Other bases, such as sodiumhydroxide and other hydroxides of alkali metals, can also be used. Incertain brines, it may be beneficial to remove boron from the productstream at this point process by known means, such as by precipitation,solvent extraction, or ion exchange.

Lithium chloride-rich stream 24 may have a concentration of betweenabout 1% and 42% by weight, preferably greater than about 10% by weight,more preferably greater than about 25% by weight. In alternateembodiments, lithium chloride-rich stream 24 may have a concentration ofgreater than about 10% by weight.

In certain embodiments, lithium chloride containing solution 24 canoptionally undergo a purification or concentration step prior to beingprovided to electrolytic process 32. Methods for the isolation andpurification of lithium chloride from brines, including geothermalbrines, are known in the art, for example, as described in U.S. Pat.Nos. 4,036,713 and 5,951,843, each of which is herein incorporated byreference in its entirety.

Optionally, the process can include steps for increasing theconcentration of the lithium chloride stream. Specifically, lithiumconcentration means 26 can be utilized for the removal of a portion ofthe water in the lithium chloride stream, for example, by evaporation,thereby producing a more concentrated lithium chloride solution 30.Exemplary concentration means can include solvent extraction,electrodialysis, reverse osmosis, steam evaporation, or solarevaporation. Water 28 removed from the lithium chloride containingsolution can be recovered, for example by evaporation and subsequentcondensation, and resupplied to intercalated lithium absorbent column(s)18, or can be supplied to any other step in this or an associatedprocess that requires the supply of water. Alternatively, water 28 canbe supplied to a geothermal well. In embodiments employing aconcentration step, overall concentration of concentrated lithiumchloride-rich solution 30 can be increased to greater than 25% lithiumchloride by weight, preferably up to about 40% lithium chloride byweight. As the concentration of the lithium chloride increases, thesodium chloride present will precipitate as halite.

Concentrated lithium chloride-rich solution 30 can be supplied toelectrochemical cell 32, which includes at least one anode, one cathodeand a permeable membrane, for the electrochemical preparation of lithiumhydroxide. Electrochemical cells suitable for large scale production arecommercially available from companies, such as, Ineos, DeNora, ChlorineEngineers, and Asahi Glass, to name a few. Specifically, chloride ionsare oxidized to chlorine at the anode and water is reduced to hydroxideions and hydrogen gas at the cathode. Preferably, concentrated lithiumchloride-rich solution 30 is substantially free of other ions,particularly ions that may interfere with the electrochemical reaction.Optionally, a lithium chloride-rich stream can supplied directly to theelectrochemical reaction, without being first being subjected to thesilica management and lithium ion sequestration steps, provided that thelithium chloride-rich stream is substantially free of non-lithium ions,particularly non-lithium ions that may interfere with theelectrochemical reaction, In certain embodiments, the concentration ofsodium and/or potassium ions in concentrated lithium chloride-richsolution 30 is less than about 5% by weight, preferably less than about3% by weight. Cations such as iron, calcium, magnesium, and the like, ifat all present, preferably have a total concentration of less than about0.001% by weight, more preferably less than about 0.005% by weight, andeven more preferably less than about 0.00001% by weight. Higherconcentrations of the interfering ions does not necessarily precludeoperation of the electrochemical cell, but instead may reduce theoverall life of the cell components and/or the overall effectiveness ofthe reaction.

Similar to that which is noted above with respect to the presence ofnon-lithium interfering cations, electrochemical cell 32 preferably hasa total non-chloride anion content of less than about 5% by weight,preferably less than about 3% by weight, and even more preferably lessthan about 1% by weight.

The cathode of electrochemical cell 32 can be any suitable material,including nickel, catalyzed nickel mesh, stainless steel, coatedstainless steel, mild steel, and the like. Other exemplary catalysts caninclude mixed ruthenium compounds, platinum and other similar compoundsthat have low hydrogen over potential. The total area of the cathode canbe adjusted based upon reactor size and desired production. Thecatholyte feed of the electrochemical cell 32 can be any suitablematerial having sufficient ions to carry a current. While water may beemployed, and in certain embodiments, the addition of lithium carbonateor lithium hydroxide may be beneficial to the operation of the cell.

The anode of electrochemical cell 32 can be any suitable material, suchas titanium mesh coated with ruthenium oxide, titanium mesh coated withplatinum, carbon, or the like. Preferably, the anode is a dimensionallystable anode, allowing for reduced power consumption. Dimensionallystable titanium anodes are particularly well-suited for chlorineenvironments as the titanium substrate is resistant to corrosion. Thetotal area of the anode can be adjusted based upon reactor size anddesired production. The anolyte of electrochemical cell 32 can be anysuitable material, including a lithium chloride solution having aconcentration of between of about 1% by weight to saturation, preferablybetween 5% and 40% by weight, more preferably between about 10% and 35%by weight.

The materials for construction of electrochemical cell 32 can be anymaterial that is chemically resistant to chlorine, activated chlorine,oxygenated chlorine species, and other dissolved species that may existin brine solutions. Exemplary materials for the construction ofelectrochemical cell 32 include polytetrafluoroethylene (PTFE),polyvinylidene fluoride (PVDF), HALAR (alternating co-polymers ofethylene and chlorotrifluoroethylene (CTFE)), and other fluorinated orpartially fluorinated.

The membrane of electrochemical cell 32 can be any suitablesemi-permeable cation selective membrane that selectively passes cationsand inhibits the passage of anions. Such membranes are known in the art.One exemplary membrane is Nafion (E.I. DuPont de Nemours & Co.),particularly the Nafion 300, 400 and 900/9000 series of materials. Othersuitable membranes can be supplied by Flemion, however any suitablemembrane material can be used provided the material is chemicallyresistant to both chlorine and lithium hydroxide. The membrane may beplaced between the anolyte being electrolyzed and the catholyte.

In certain embodiments, the process can optionally include one or morefilter or separation-purification step prior to the step of supplyingconcentrated lithium chloride solution 30 or brine to electrochemicalcell 32.

During operation of electrochemical cell 32, a current density ofbetween about 500 and 10,000 A/m² can be applied at a voltage of betweenabout 1.5 and 5 volts. Preferably, a current density of between about2000 and 7000 A/m² is applied.

Electrochemical cell 32 may be operated at a temperature of betweenabout 60° and 100° C., preferably between about 70° and 95° C., and morepreferably between about 90° and 95° C. Cell 32 can be operated atatmospheric pressure, or slightly above atmospheric pressure.

Operation of electrochemical cell 32 produces lithium hydroxide insolution, and also evolves chlorine and hydrogen gas by products, whichcan be removed from the electrochemical cell via lines 34 and 35,respectively.

The efficiency of electrochemical cell 32 is at least about 60%,preferably at least about 70%, more preferably at least about 80%, morepreferably at least about 90%, more preferably at least about 95%, andeven more preferably at up to about 99.9%. The electrolysis can beoperated continually until the lithium hydroxide content reaches about17% by weight, at which time the lithium hydroxide solution may beremoved and supplied to a carbonation reactor. At lithium hydroxideconcentrations greater than about 17% by weight, the lithium hydroxidein solution can begin to precipitate. Electrochemical cell 32 can alsobe operated under conditions designed to produce lower concentrationlithium hydroxide solutions and the lower concentration lithiumhydroxide solution can be recycled to and from the carbonation reactor.In certain embodiments, electrochemical cell 32 can also include a feedline (not shown) for supplying water, low concentration lithiumhydroxide, low concentration lithium carbonate, or combinations thereofto the cell.

Lithium hydroxide solution 36 is supplied from electrochemical cell 32to carbonation reactor/absorber 38 and can be contacted with carbondioxide gas 44, for example, in an up-flow fashion. Carbonationreactor/absorber 38 can include a series of trays or other like meansthat are designed to allow lithium hydroxide 36 to be supplied to thetop of the reactor and flow in a downward fashion through the reactor,thereby contacting up-flowing carbon dioxide gas 44, which can beintroduced near the bottom of carbonation reactor/absorber 38. Inalternate embodiments, carbonation reactor/absorber 38 can includevarious mixing means designed to facilitate mixing of liquids and gases.Optionally, carbonation reactor/absorber 38 can be a jacketed batchreactor having thermostatic heating. The reaction produces lithiumcarbonate solid. The concentration of the lithium carbonate slurry ispreferably at least about 1.5% by weight lithium carbonate, morepreferably at least about 6% by weight lithium carbonate. Carbon dioxidecan be captured and recycled to carbonation reactor/absorber 38 via line42.

In certain embodiments, the lithium carbonate can produced by reactionof lithium hydroxide with sodium carbonate in water, wherein the mixtureis heated, preferably to a temperature of between about 90° C. and 95°C., with stirring. The reaction produces solid lithium carbonate and asodium chloride solution, wherein the sodium chloride solution can beseparated by filtration from the desired lithium carbonate solids.

Lithium carbonate solution 40 can be supplied to filtration means 46,which is operable to separate lithium carbonate containing slurry 40into water stream 52, which may optionally be resupplied to thefiltration means, and solid lithium carbonate product 50. Filtrationmeans 46 can, for example, include a series of screens or filters andwater supply 48. Optionally, water can be recycled to the process vialine 52. Optionally, lithium carbonate can be concentrated from theslurry by centrifugation or decantation thickening. Water collectedduring the separation of the solids from the slurry via filtration means46 can be supplied to the electrochemical cell, or may be supplied to ageothermal well or reservoir. In certain embodiments, lithium carbonatesolid can be retained on a band filter and supplied to a wash step,wherein hot water, preferably having a temperature of between about 90°C. and 95° C. is used to wash the solids. In certain embodiments, theaqueous solution collected via filtration means 46 can have a pH ofgreater than about 9, most likely having a pH between about 10-12.Alternatively, sufficient acid can be added to the aqueous solution toachieve a pH of between about 5 and 8.5, and the acidified water canthen be supplied to the intercalated lithium absorbent column(s).Alternatively, the solution can be returned directly to the cathode sideof the electrolysis cell without prior neutralization.

The solid lithium carbonate 50 is supplied to a drying station 54, whichcan optionally include heating means, as well as lines for supplyingnitrogen or other inert gases to the chamber. Dried lithium carbonateproduct 56 can then be collected, packaged and transported for furtheruse.

Referring now to FIG. 4, an alternate embodiment for the production oflithium carbonate is provided. Lithium chloride stream 30 is provided bythe process described above and as shown in FIG. 3. To electrochemicalcell 32, which is as described above, sodium chloride stream 60 isprovided. Sodium chloride stream 60 is then subjected to electrolysis toproduce sodium hydroxide stream 62 and chlorine and hydrogen gases 64.Reaction conditions for the production of sodium hydroxide byelectrolysis of sodium chloride are known in the art.

In certain embodiments, the efficiency of the electrolysis of sodiumchloride is at least about 70%, alternatively at least about 80%,alternatively at least about 90%, or alternatively at least about 95%.In certain embodiments, sodium hydroxide solution 62 is produced in at aconcentration of at least about 10% by weight, more preferably at leastabout 30% by weight, and most preferably about 35% by weight.

Chlorine and hydrogen gases 64, 65 from electrochemical cell 32 can becombusted and scrubbed with water to generate hydrochloric acid, whichmay be used within the process, or alternately may be purified,compressed, and sold commercially.

Sodium hydroxide stream 62 is supplied to carbonation reactor/absorber38, wherein the sodium hydroxide stream is contacted with carbon dioxidesteam 44, for example, in an up-flow fashion. Carbonationreactor/absorber 38 can include a series of trays, designed to allowsodium hydroxide stream 62 to be supplied to the top of the reactor andflow in a downward fashion through the reactor, thereby contacting upflowing carbon dioxide gas 44, which can be introduced near the bottomof the reactor, to produce sodium carbonate solution or slurry 66. Inalternate embodiments, carbonation reactor/absorber 38 can includevarious mixing means designed to facilitate mixing of liquids and gases.The concentration of the solution is preferably at least 15% by weightsodium carbonate, more preferably at least 25% by weight sodiumcarbonate. Carbon dioxide can be captured and recycled to carbonationreactor/absorber 38 via line 42.

Sodium carbonate solution 66 is supplied to reaction vessel 68 whereinthe solution is contacted with lithium chloride solution 30 to produceslurry 70, which includes lithium carbonate and sodium chloridesolution. The step of contacting sodium carbonate solution 66 andlithium chloride solution 30 in the reaction vessel can be at atemperature greater than about 60° C., preferably greater than about 80°C., and even more preferably between about 90° C. and 95° C. In certainembodiments, reaction vessel 68 can be a stirred tank reactor.Alternatively, reaction vessel 68 can be a standard crystallizer.Lithium carbonate is present as a precipitate, while sodium chlorideremains in aqueous solution.

Slurry 70, which includes solid lithium carbonate and aqueous sodiumchloride, is supplied to separator 72, which can include various meansfor the separation of solids from liquids including, for example,centrifuge, settling tank, filters, screens, and the like, to producelithium carbonate product stream 74 and sodium chloride brine solution76. In order to attain improved product quality, the lithium carbonatecan be treated to remove sodium, potassium, and/or chloride ions trappedin the interstitial space of the lithium carbonate precipitate, such asby washing with water, preferably hot water, or by like means. Incertain embodiments, separator means 72 can be a band filter or rotarydrum, and can optionally be fed through a counter current wash systemfor the removal of residual sodium chloride. Separator means 72 can alsoinclude water inlet 72 and outlet 76 for the washing of the separatedsolid lithium carbonate. Separator means 72 can also include means fordrying and/or the removal of water from the solid lithium carbonate,including for example, centrifuge, heaters, blowers, presses, and thelike. Separator means 72 can include a vacuum filter for removal ofwater. In certain embodiments, it is desirable to optimize the washingstep to both maximize purity of the lithium carbonate while minimizingthe amount of water used for washing. Sodium chloride solution 76 can berecycled to electrochemical cell 32 for electrolysis. Lithium carbonateproduct 74 can have a moisture content of less than about 5% by weight,preferably less than about 2% by weight, and even more preferably lessthan about 0.5% by weight.

The brine solution 76 from separator means 72 can include sodiumchloride and lithium carbonate. Generally, depending upon the amount ofwater utilized in the process and during the wash process, the ratio ofsodium chloride to lithium carbonate is at least about 20:1, morepreferably at least about 25:1, and even more preferably at least 30:1.In certain embodiments, the ratio of sodium chloride to lithiumcarbonate in the brine solution can be about 35:1.

In certain embodiments, brine solution 76 can be acidified withhydrochloric acid (not shown) to a pH of less than about 4, preferablyabout 3, and recycled to electrochemical cell 32. The hydrochloric acidcan be supplied from electrochemical cell 32.

The lithium carbonate production method proposed in FIG. 4 isadvantageous because the process eliminates, or nearly eliminates, theproduction of waste products. Specifically, in certain embodiments, therecycle of unused metal salts, for example sodium chloride, and carbondioxide, the overall yield can be quantitative or nearly quantitative.

Referring now to FIG. 5, another alternate embodiment for the productionof lithium carbonate is provided. The method is a single step processwherein sodium carbonate is produced and reacted with recovered lithiumchloride, however may require additional input and produces a wastelithium chloride stream that may include small amounts of lithiumcarbonate entrained therein.

A lithium chloride stream is provided as described above and as shown inFIG. 3. To electrochemical cell 32 sodium chloride stream 60 isprovided. Sodium chloride stream 60 is subjected to electrolysis toproduce sodium hydroxide 62 and chlorine and hydrogen gases 64, 65,respectively.

Sodium hydroxide stream 62 is supplied to mixer 80, wherein the sodiumhydroxide stream is combined and mixed with lithium chloride stream 30.Mixing of sodium hydroxide stream 62 and lithium chloride stream 30 canbe by known means, such as by agitators or mixers, with ultrasonicwaves, or by the like. Mixer 80 produces mixed stream 82, which includessodium hydroxide and lithium chloride in aqueous solution. In certainembodiments, it may be preferred that lithium chloride steam 30 has aconcentration of at least about 20% by weight, more preferably at leastabout 28% by weight, and even more preferably about 42% by weight.Similarly, in certain embodiments, it may be preferred that sodiumhydroxide stream 62 has a concentration of at least about 15% by weight,more preferably at least about 25% by weight, and even more preferablyabout 35% by weight.

Mixed stream 82 is supplied to carbonation reactor/absorber 84, whichcan include a series of trays, designed to allow the mixed stream, whichincludes lithium chloride and sodium hydroxide, to be supplied to thetop of the reactor and flow in a downward fashion through the reactor,thereby allowing the mixed stream to sufficiently contact up-flowingcarbon dioxide gas 44, which can be introduced near the bottom of thereactor via line 22, to produce a lithium carbonate slurry 90.Preferably, carbonation reactor/absorber 84 is maintained at atemperature of between about 90° C. and 100° C. In alternateembodiments, reactor 84 can include various mixing means designed tofacilitate mixing of liquids and gases. The concentration of the lithiumcarbonate is preferably at least 15% by weight, more preferably at least25% by weight lithium carbonate. Carbon dioxide can be recycled tocarbonation reactor 38 via line 42.

Lithium carbonate solution 90 is supplied to separation vessel 92wherein solid lithium carbonate is produced via line 94. A solution thatincludes sodium chloride and possibly a small amount of lithiumcarbonate is produced as stream 96.

Sodium carbonate solution 90, which includes solid lithium carbonate andaqueous sodium chloride, is supplied to separator means 92, which caninclude various means for the separation of solids from liquidsincluding, for example, centrifuge, settling tank, filters, screens, andthe like. Separator means 92 can also include water inlets and outlets(not shown) for the washing of the separated solid lithium carbonate.Separator means 72 can also include means for drying and/or the removalof water from the solid lithium carbonate, including for example,centrifuge, heaters, blowers, presses, and the like. A solid sodiumcarbonate product is collected via line 94. Optionally, a portion ofsodium chloride stream 96 can be recycled to electrochemical cell 32.Optionally, the sodium chloride solution can be recycled to the washingstep of the lithium extraction media. In certain embodiments, the sodiumchloride required for the process can be generated by the selectivecrystallization of sodium chloride from the geothermal, Smackover, orother brine.

Referring to FIG. 10, in one embodiment of the present method, lithiumchloride containing solution 10 is provided. As noted above, lithiumchloride containing solution 10 can be obtained from a variety ofsources, including geothermal brines. The lithium chloride containingsolution can be supplied to silica management step 12, which operates tosignificantly reduce the amount of silica present in lithium chloridecontaining solution 10, to produce silicate precipitate 16 andsilica-lean lithium chloride containing solution 14. After silica hasbeen removed, the silicon concentration in silica-lean lithium chloridecontaining solution 14 is less than about 150 ppm, preferably theconcentration is less than about 100 ppm, more preferably theconcentration is less than about 50 ppm, and even more preferably theconcentration is less than about 25 ppm. In certain embodiments, theconcentration of silicon in silica-lean lithium chloride containingsolution 14 is less than about 20 ppm, alternatively less than about 10ppm, alternatively less than about 5 ppm, alternatively less than about3 ppm, or alternatively less than about 1 ppm. In certain embodiments,it is understood that the silica concentration is desired to be as smallas possible. It is understood that the silica management step isoptional and may be omitted from the process for brines that do notinclude silica, or brines that have a substantially low initial silicaconcentration.

In certain embodiments, silica management step 12 can include the stepof contacting lithium chloride containing solution 10 with activatedalumina to remove at least a portion of the silica present. Alumina thatincludes silica bound thereto can be regenerated by contacting thealumina with sodium hydroxide. Alternatively, the lithium chloridecontaining solution can be contacted with aluminum chloride, which isconverted to aluminum hydroxide, and can be used to precipitate silicapresent in the lithium chloride containing stream. In a furtherembodiment, iron (II) that may be present in certain lithium containingbrines can be oxidized with an oxidant, such as air, hypochlorite,hydrogen peroxide, oxygen, ozone, or a like oxidizing agent, to generateiron (III) chloride, which after adjustment of the pH to above about 5,from an initial pH of about 2.5 to 3.5, will precipitate ferrichydroxide. The ferric hydroxide can adsorb silica from the lithiumcontaining brine. In a preferred embodiment, the pH is adjusted tobetween about 5 and 6 to induce precipitation of silica and iron. Inalternate embodiments, the pH is adjusted to above at least about 4.5 toinduce precipitation of silica and iron. In certain embodiments, it ispreferred the pH is not increased above about 6, to prevent theprecipitation of other ionic species present in the lithium containingbrine. In yet another embodiment, iron (II) can be added to the lithiumchloride containing solution and oxidized by known means to iron (III),such as with by contacting the iron (II) with an oxidant, such as air,oxygen, ozone, hypochlorite, hydrogen peroxide, or other suitableoxidizing agent. Contacting silica present in the lithium chloridecontaining solution with the iron (III) compound forms a precipitatewhen the pH is adjusted to between about 4.5 and 6 with the addition oflime or similar base. It a preferred embodiment, the pH is adjusted tobetween about between about 5 and 6. In alternate embodiments, the pHmust be adjusted to above at least about 4.5 for the silica and iron toprecipitate. In certain embodiments, it is preferred the pH is notincreased above about 6, to prevent the precipitation of other ionicspecies.

In addition, silica management step 12 can include any known means forremoving a portion of the silica present in the feed stream, while atthe same time maintaining the initial concentration of lithium. In oneembodiment, lithium chloride containing solution 10 can be contactedwith aluminum chloride, iron chloride, aluminum hydroxide, or the like,to form a precipitate with the silicon dioxide. Contacting can befacilitated by known means, such as a mixing device. Solid silicaprecipitate 16 removed from lithium chloride containing solution 10 canbe collected and removed from the mixing or like device, by known means,such as screening or filtering, to yield lithium chloride containingstream 14 that is substantially free of silica.

As known in the art, various membranes can be used to selectively removespecific undesired ions from lithium containing solution 14.

Silica-lean lithium chloride containing stream 14, which issubstantially free of silica (measured as SiO₂), can be supplied tolithium chloride isolation step. In certain embodiments, silica-leanlithium chloride containing stream 14 can be supplied to at least oneintercalated lithium absorbent column 18, which can be configured toabsorb and isolate lithium chloride from the silica-lean lithiumchloride containing solution, while at the same time allowing otherions, such as calcium, magnesium, and/or sodium, or the like, to passwith water stream 22, through the use of a selective molecular sieve,membrane, or other like materials. In embodiments that include more thanone intercalated lithium absorbent column for the extraction of lithium,a major portion of the lithium is removed in the first intercalatedlithium absorbent column, with any subsequent “polishing” intercalatedlithium absorbent columns being used to minimize overall lithium lossduring the recovery process.

In certain embodiments, the intercalated lithium absorbent column can beoperated as follows. Lithium alumina intercalate particles having anaverage diameter of between about 100 and 650 μm, preferably betweenabout 300 and 450 μm, can be combined with a saturated sodium chloridesolution that includes approximately 200 ppm lithium chloride to preparea slurry, which can then be added to the column. The column may bejacketed, insulated or may include means to provide heating or coolingto the column. The column may include a method of distributing liquidand support for the extraction media and can include fritted ends havinga pore size of between approximately 25 and 50 μm, although other likemeans, such as supports of glass wool or perforated plates, can also beused instead of fitted ends. For the present invention, the operatingtemperature of the column can be maintained at a temperature that isgreater than room temperature, alternatively at a temperature aboveabout 70° C., preferably between about 95° C. and 110° C.

The column is maintained wet and is unloaded before the first use bycirculating at least about 1 bed volume, preferably about two bedvolumes, of deionized water 20 that includes approximately 1000 ppmlithium chloride, at a flow rate of between approximately 1 and 4 bedvolumes/hour, preferably between about 1.5 and 2.5 bed volumes/hour. Thecolumn is then contacted with approximately one bed volumes of saturatedsodium chloride solution containing approximately 200 ppm lithiumchloride is then run.

During loading of the column (i.e., during the step of capturing desiredlithium chloride), high ionic strength solution 14 containing lithiumchloride is supplied to column 18 and the lithium concentration of theeffluent at column outlet 22 is measured to determine the point at whichthe column becomes saturated with the lithium chloride. During thelithium ion capture step, the lithium concentration at outlet 22 remainsfairly constant and relatively low, for example, approximately 0 and 100ppm. The point at which column 18 reaches or nears the point ofsaturation with lithium ions, however, the concentration of the lithiumin the effluent increases, thus indicating that the column has eitherlittle or no capacity for additional lithium ions. Upon reaching thispoint of saturation, flow of the solution that includes lithium chlorideto column 18 stopped, and the column is flushed with between about 1 and8 bed volumes of deionized water, preferably between about 1 and 2.5 bedvolumes, and most preferably between about 1 and 1.5 bed volumes, toproduce a lithium chloride-rich stream 24. It is understood that theapparatus can include various valves and control devices for controllingthe flow of the lithium containing solution or the wash solution to thecolumn.

In certain embodiments, after loading of the column, but beforecollection of the captured lithium chloride, the column may be flushedwith about 1 bed volume of a 26% saturated sodium chloride solution thatincludes about 200 ppm lithium chloride.

After the removal of lithium chloride from the lithium containing feedstream during the lithium chloride isolation step, intercalated lithiumabsorbent columns 18 can be regenerated and the lithium chloriderecovered therefrom. Specifically, at least about 0.5 equivalents ofwash water 20 may be supplied to column(s) 18 to remove absorbed lithiumchloride and produce lithium chloride rich solution 24. In certainembodiments, between about 1 to 2 equivalents of wash water 20, or moreequivalents, may be used during the regeneration of the columns. Incertain embodiments, the wash water may include lithium ions for theregeneration of the columns. Optionally, low ionic strength liquids,such as alcohols and water/alcohol mixtures can be used to regeneratethe columns. In general, the amount of water utilized for lithiumchloride recovery from the column is minimized by recycling productstreams to maximize lithium content, without reducing the capacity ofthe extracting media.

Optionally, a purification step can be employed to remove calcium,magnesium, or other divalent ions such as zinc and manganese that may bepresent in lithium chloride-rich stream 24. Removal of calcium,magnesium, and/or other alkaline earth metals can be achieved by knownmeans, such as, by increasing the pH and treating the solution with ionexchange, preferably using selective chelating ion exchange resins, orby the addition of a base, such as lime, sodium hydroxide, lithiumhydroxide, or the like, followed by the addition of lithium carbonate,sodium carbonate, potassium carbonate, ammonium carbonate, or othersuitable carbonate, which can precipitate magnesium and iron hydroxide,as well as calcium carbonate. In alternate embodiments, ion exchangemeans can be employed to facilitate the removal of calcium, magnesium,and/or other alkaline earth metals. Other bases, such as sodiumhydroxide and other hydroxides of alkali metals, can also be used. Incertain brines, it may be beneficial to remove boron from the productstream at this point process by known means, such as by precipitation,solvent extraction, or ion exchange.

Lithium chloride-rich stream 24 may have a concentration of betweenabout 1% and 42% by weight, preferably greater than about 10% by weight,more preferably greater than about 25% by weight. In alternateembodiments, lithium chloride-rich stream 24 may have a concentration ofgreater than about 10% by weight.

In certain embodiments, lithium chloride containing solution 24 canoptionally undergo a purification or concentration step prior to beingprovided to electrolytic process 32. Methods for the isolation andpurification of lithium chloride from brines, including geothermalbrines, are known in the art, for example, as described in U.S. Pat.Nos. 4,036,713 and 5,951,843, each of which is herein incorporated byreference in its entirety.

Optionally, the process can include steps for increasing theconcentration of the lithium chloride stream. In certain embodiments,the concentration process can include solvent extraction of lithiumchloride containing solution 24. The solvent extraction process caninclude the steps of extracting the lithium chloride containing solution24 with an organic solvent that includes a compound that is designed toselectively remove lithium from the lithium containing solution. Incertain embodiments, lithium chloride may be extracted by the extractioncompound. As shown in FIG. 11, lithium chloride containing solution 24is provided to extraction column 104. Extraction column 104 can be apulsed column, a separation funnel, a mixer settler consisting of inlinemixing, agitated vessels and a settling tank, or like equipment that isconfigured for liquid-liquid extraction processes. Lithium chloridecontaining solution 24 can have a lithium chloride concentration of upto about 10%, alternatively less than about 5, alternatively betweenabout 2 and 4%. In extraction column 104, lithium chloride containingsolution 24 is contacted with an organic phase that is supplied via line124. The organic phase can include an extracting agent and a carriersolvent. Exemplary extracting agents generally include, but are notlimited to, crown ethers, aza crown ethers, and phosphonic acids.Exemplary compounds can include 4-benzoylacyl-5-pyrazolone,4-perfluoroacyl-5-pyrazolone, trioctylphosphine oxide (TOPO),bis(2,2,4-trimethylpentyl)phosphinic acid, CYANEX 272 extractant, CYANEX923 extractant (which is a mixture that includes 4 trialkylphosphines,including R₃P(O), R₂R′P(O), RR′₂P(O), and R′₃P(O), wherein R is ann-octyl substituent (CH₃(CH₂)₇) and R′ is an n-hexyl substituent(CH₃(CH₂)₅), bis(2,2,4-trimethylpentyl)dithiophosphinic acid, CYANEX301, lipophilic 12-crown-4, monoaza 15-crown-5, lipophilic 14-crown-4,lipophilic monoaza 14-crown-4, chromogenic 14-crown-4, monoaza12-crown-4, monoaza 13-crown-4, monoaza 14-crown-4, and the like.Certain preferred extracting agents include compounds that demonstrateselectivity for lithium over other alkali ions, for example sodium, suchas monoaza 14-crown-4. Exemplary carrier solvents for the extractingagent can include toluene, benzene, xylene, Aromatic 100 (also known asType 1 Light Aromatic Solvent Naphtha), Aromatic 150 (also known at TypeII Heavy Aromatic Solvent Naphtha), cyclohexane, dioxane, kerosene,Escaid 110 diluent (having a paraffin content of greater than about99.5%), Kermac 470B diluent, Orform SX80 (having a composition of about55% by vol. paraffins, 20% by vol. alkyl aromatics, and 23% by vol.naphthenes), LINPAR 1416 (a straight chain hydrocarbon saturated mixtureof hydrocarbons between C₁₄ and C₁₆), and other like compounds, andmixtures thereof. In general, the carrier solvents can be de-aromatizedhydrocarbons having less than about 0.5% aromatics or can be diluentshaving between 17-23% by volume aromatics. Typically, the paraffincontent of the carrier solvent is about 40% by volume cycloparaffins.Considerations in selecting the carrier solvent include flash point andenvironmental concerns, such as disposal. Typically, the aromaticcontent of the carrier solvent have the following effects on solventextraction of metals: increased solubility of the metal-extractantcomplex in the organic phase; as an equilibrium modifier; and toinfluence selectivity.

In contacting the lithium chloride containing solution and the organicphase, lithium ions are captured by the extracting agent. The organicand aqueous phases are separated from extraction column 104 to producean aqueous phase that is removed via line 106 and an organic phase thatis supplied via line 108 to scrubbing column 110. The aqueous phase inline 106 can include a small concentration of lithium chloride,typically less than about 2%, alternatively less than about 1000 ppm,and preferably less than about 1000 ppm. The aqueous phase can beconcentrated and HCl removed by reverse osmosis, evaporation,perevaporation, osmosis, or other suitable concentration process, oralternatively can be supplied directly to the lithium capture step. Incertain embodiments, the aqueous phase may need to be neutralized priorto being supplied to the lithium capture step.

The organic phase is supplied to scrubbing column 110 via line 108 andis contacted with a scrub solution that is supplied via line 114 andcontacts the organic phase in a counter current flow. The scrubbingsolution can be an aqueous acid solution, typically a dilute strongacid, such as HCl, HBr, H₂SO₄, HNO₃, or a like strength acid, typicallyat a concentration of between about 0.1 M and 1 M. Alternatively, aconcentrated weak acid could also be used. Scrubbing column 110 producesan aqueous phase that is removed via line 112 and can optionally besupplied to the brine solution, provided there is no significant changein the pH (i.e., pH does not increase or decrease by more than about0.5). In certain embodiments, the aqueous phase that is removed via line112 can be neutralized prior to being supplied to the brine. A scrubbedorganic phase that includes the extracting agent and captured lithiumions, as well possibly including a minor amount of free sodium ions, isremoved from scrubbing column 112 via line 116 and supplied to strippingcolumn 118. In certain embodiments, the scrubbing step is optional.

Scrubbed organic phase supplied via line 116 to stripping column 118 iscontacted with concentrated HCl or H₂SO₄, for example 20-36% HCl, in acounter current flow to release lithium ions from the extracting agent.A concentrated lithium chloride-rich solution having a concentration ofbetween about 20 and 40%, alternatively greater than about 30%, isproduced and removed via line 30. An recovered organic phase thatincludes the extracting agent and carrier solvent is removed fromstripping column 118 via line 124 and can be supplied to extractioncolumn 104.

Concentrated lithium chloride-rich solution 30 can be supplied toelectrochemical cell 32, which includes at least one anode, one cathodeand a permeable membrane, for the electrochemical preparation of lithiumhydroxide. Electrochemical cells suitable for large scale production arecommercially available from companies, such as, DeNora, ChlorineEngineers, and Asahi Glass, to name a few. Specifically, chloride ionsare oxidized to chlorine at the anode and water is reduced to hydroxideions and hydrogen gas at the cathode. Preferably, concentrated lithiumchloride-rich solution 30 is substantially free of other ions,particularly ions that may interfere with the electrochemical reaction.Optionally, a lithium chloride-rich stream can supplied directly to theelectrochemical reaction, without being first being subjected to thesilica management and lithium ion sequestration steps, provided that thelithium chloride-rich stream is substantially free of non-lithium ions,particularly non-lithium ions that may interfere with theelectrochemical reaction, In certain embodiments, the concentration ofsodium and/or potassium ions in concentrated lithium chloride-richsolution 30 is less than about 5% by weight, preferably less than about3% by weight. Cations such as iron, calcium, magnesium, and the like, ifat all present, preferably have a total concentration of less than about0.001% by weight, more preferably less than about 0.005% by weight, andeven more preferably less than about 0.00001% by weight. Higherconcentrations of the interfering ions does not necessarily precludeoperation of the electrochemical cell, but instead may reduce theoverall life of the cell components and/or the overall effectiveness ofthe reaction.

Similar to that which is noted above with respect to the presence ofnon-lithium interfering cations, electrochemical cell 32 preferably hasa total non-chloride anion content of less than about 5% by weight,preferably less than about 3% by weight, and even more preferably lessthan about 1% by weight.

The cathode of electrochemical cell 32 can be any suitable material,including nickel, catalyzed nickel mesh, stainless steel, coatedstainless steel, mild steel, and the like. Other exemplary catalysts caninclude mixed ruthenium compounds, platinum and other similar compoundsthat have low hydrogen over potential. The total area of the cathode canbe adjusted based upon reactor size and desired production. Thecatholyte feed of the electrochemical cell 32 can be any suitablematerial having sufficient ions to carry a current. While water may beemployed, and in certain embodiments, the addition of lithium carbonateor lithium hydroxide may be beneficial to the operation of the cell.

The anode of electrochemical cell 32 can be any suitable material, suchas titanium mesh coated with ruthenium oxide, titanium mesh coated withplatinum, carbon, or the like. Preferably, the anode is a dimensionallystable anode, allowing for reduced power consumption. Dimensionallystable titanium anodes are particularly well-suited for chlorineenvironments as the titanium substrate is resistant to corrosion. Thetotal area of the anode can be adjusted based upon reactor size anddesired production. The anolyte of electrochemical cell 32 can be anysuitable material, including a lithium chloride solution having aconcentration of between of about 1% by weight to saturation, preferablybetween 5% and 40% by weight, more preferably between about 10% and 35%by weight.

The materials for construction of electrochemical cell 32 can be anymaterial that is chemically resistant to chlorine, activated chlorine,oxygenated chlorine species, and other dissolved species that may existin brine solutions. Exemplary materials for the construction ofelectrochemical cell 32 include polytetrafluoroethylene (PTFE),polyvinylidene fluoride (PVDF), HALAR (alternating co-polymers ofethylene and chlorotrifluoroethylene (CTFE)), and other fluorinated orpartially fluorinated.

The membrane of electrochemical cell 32 can be any suitablesemi-permeable cation selective membrane that selectively passes cationsand inhibits the passage of anions. Such membranes are known in the art.One exemplary membrane is Nafion (E.I. DuPont de Nemours & Co.),particularly the Nafion 300, 400 and 900/9000 series of materials. Othersuitable membranes can be supplied by Flemion, however any suitablemembrane material can be used provided the material is chemicallyresistant to both chlorine and lithium hydroxide. The membrane may beplaced between the anolyte being electrolyzed and the catholyte.

In certain embodiments, the process can optionally include one or morefilter or separation-purification step prior to the step of supplyingconcentrated lithium chloride solution 30 or brine to electrochemicalcell 32.

During operation of electrochemical cell 32, a current density ofbetween about 500 and 10,000 A/m² can be applied at a voltage of betweenabout 1.5 and 5 volts. Preferably, a current density of between about2000 and 7000 A/m² is applied.

Electrochemical cell 32 may be operated at a temperature of betweenabout 60° and 100° C., preferably between about 70° and 95° C., and morepreferably between about 90° and 95° C. Cell 32 can be operated atatmospheric pressure, or slightly above atmospheric pressure.

Operation of electrochemical cell 32 produces lithium hydroxide insolution, and also evolves chlorine and hydrogen gas by products, whichcan be removed from the electrochemical cell via lines 34 and 35,respectively.

The efficiency of electrochemical cell 32 is at least about 60%,preferably at least about 70%, more preferably at least about 80%, morepreferably at least about 90%, more preferably at least about 95%, andeven more preferably at up to about 99.9%. The electrolysis can beoperated continually until the lithium hydroxide content reaches about17% by weight, at which time the lithium hydroxide solution may beremoved and supplied to a carbonation reactor. At lithium hydroxideconcentrations greater than about 17% by weight, the lithium hydroxidein solution can begin to precipitate. Electrochemical cell 32 can alsobe operated under conditions designed to produce lower concentrationlithium hydroxide solutions and the lower concentration lithiumhydroxide solution can be recycled to and from the carbonation reactor.In certain embodiments, electrochemical cell 32 can also include a feedline (not shown) for supplying water, low concentration lithiumhydroxide, low concentration lithium carbonate, or combinations thereofto the cell.

Lithium hydroxide solution 36 is supplied from electrochemical cell 32to carbonation reactor/absorber 38 and can be contacted with carbondioxide gas 44, for example, in an up-flow fashion. Carbonationreactor/absorber 38 can include a series of trays or other like meansthat are designed to allow lithium hydroxide 36 to be supplied to thetop of the reactor and flow in a downward fashion through the reactor,thereby contacting up-flowing carbon dioxide gas 44, which can beintroduced near the bottom of carbonation reactor/absorber 38. Inalternate embodiments, carbonation reactor/absorber 38 can includevarious mixing means designed to facilitate mixing of liquids and gases.Optionally, carbonation reactor/absorber 38 can be a jacketed batchreactor having thermostatic heating. The reaction produces lithiumcarbonate solid. The concentration of the lithium carbonate slurry ispreferably at least about 1.5% by weight lithium carbonate, morepreferably at least about 6% by weight lithium carbonate. Carbon dioxidecan be captured and recycled to carbonation reactor/absorber 38 via line42.

In certain embodiments, the lithium carbonate can produced by reactionof lithium hydroxide with sodium carbonate in water, wherein the mixtureis heated, preferably to a temperature of between about 90° C. and 95°C., with stirring. The reaction produces solid lithium carbonate and asodium chloride solution, wherein the sodium chloride solution can beseparated by filtration from the desired lithium carbonate solids.

Lithium carbonate solution 40 can be supplied to filtration means 46,which is operable to separate lithium carbonate containing slurry 40into water stream 52, which may optionally be resupplied to thefiltration means, and solid lithium carbonate product 50. Filtrationmeans 46 can, for example, include a series of screens or filters andwater supply 48. Optionally, water can be recycled to the process vialine 52. Optionally, lithium carbonate can be concentrated from theslurry by centrifugation or decantation thickening. Water collectedduring the separation of the solids from the slurry via filtration means46 can be supplied to the electrochemical cell, or may be supplied to ageothermal well or reservoir. In certain embodiments, lithium carbonatesolid can be retained on a band filter and supplied to a wash step,wherein hot water, preferably having a temperature of between about 90°C. and 95° C. is used to wash the solids. In certain embodiments, theaqueous solution collected via filtration means 46 can have a pH ofgreater than about 9, most likely having a pH between about 10-12.Alternatively, sufficient acid can be added to the aqueous solution toachieve a pH of between about 5 and 8.5, and the acidified water canthen be supplied to the intercalated lithium absorbent column(s).Alternatively, the solution can be returned directly to the cathode sideof the electrolysis cell without prior neutralization.

The solid lithium carbonate 50 is supplied to a drying station 54, whichcan optionally include heating means, as well as lines for supplyingnitrogen or other inert gases to the chamber. Dried lithium carbonateproduct 56 can then be collected, packaged and transported for furtheruse.

In certain embodiments, rather than employing an electrolysis step,concentrated lithium chloride-rich solution 30 can be supplied directlyto a reactor (not shown) where it is contacted with sodium carbonate toform a lithium carbonate containing slurry.

Referring to FIG. 12, a procedure for the production of lithiumcontaining compounds from a lithium chloride containing solution isprovided. A lithium chloride containing stream having a concentration ofup to about 5%, alternatively between about 2 and 4%, is provided vialine 202 to a solvent extraction process, which is described above andshown in FIG. 11, to produce a concentrated lithium chloride containingstream, which can have a concentration of up to about 40%, alternativelybetween about 30 and 40%. The concentrated lithium chloride containingstream is supplied via line 206 to electrochemical cell 208, whichproduces gaseous HCl, which is removed via line 210 and a lithiumhydroxide containing stream, which is removed from the electrochemicalcell via line 212.

Line 212 can optionally include a splitter, allowing 2 or more processesto be supplied the lithium hydroxide containing stream. In oneembodiment, all or a portion of the lithium hydroxide is supplied to acarbonate reactor 218, which is supplied carbon dioxide via line 220,and operates as described herein. Lithium carbonate is removed as asolution or slurry from carbonate reactor 218 via line 222, and canoptionally be supplied to a filtration, wash, and/or drying process 224.A purified and optionally dried lithium carbonate product can becollected via line 226.

In alternate embodiments, all or a portion of the lithium hydroxidecontaining stream is supplied via line 212 to a crystallization step 214for the preparation of a LiOH.H₂O product, which can be removed from thecrystallization process via line 216. In general, the lithium hydroxidecontaining stream is supplied via line 212 to an evaporation chamber,wherein at least a portion of the water is removed to produce aconcentrated lithium hydroxide containing slurry. In certainembodiments, the lithium hydroxide containing stream can be supplied toa heat exchanger prior to being sent to the evaporating chamber. Thesolid from the slurry is recovered by known methods, such as filtration,centrifugation, hydrocyclones, or other means, or combinations thereof.In certain embodiments the solution maybe cooled prior to separation ofthe solid from the solution.

In another embodiment, an alternate process for the optionalpurification of lithium chloride-rich stream 24 can be provided toremove calcium, manganese, magnesium, or other divalent ions such aszinc that may be present in lithium chloride-rich stream 24. The processcan include the liquid-liquid of the lithium chloride-rich stream withan organic stream that includes an extraction compound that is selectivefor divalent ions. Exemplary extraction compounds include materialsproduced by Cytec, such as Cyanex® 272 (Cytec Industries, Inc., havingbis(2,4,4-trimethylpentyl) phosphinic acid as the main activeingredient), phosphinic and phosphoric acids, such as di(2-ethylhexyl)phosphoric acid, and other compounds known for having an affinity tobind divalent ions.

Exemplary carrier solvents for the extraction of divalent ions caninclude those that are described for the Isopar M (an isoparaffinichydrocarbon), LINPAR 1416 (a mixture of tetradecane, pentadecane andhexadecane), LPA Solvents and n-Paraffins (from Sasol), compoundsdisclosed above as liquid carriers for the concentration of the lithiumcontaining stream, and like compounds.

The process for the extraction of certain divalent ions, such asmanganese, magnesium, zinc, and calcium, proceeds as follows. A lithiumchloride-rich solution is provided, for example from the lithiumextraction column, and treated with an organic solvent extractionproduct. Optionally, the pH of the lithium chloride-rich stream adjustedprior to contacting lithium chloride-rich stream with the organicsolvent extraction product. After contacting the lithium chloride-richstream with the organic solvent extraction product, the two phases areallowed to separate, providing an aqueous phase and an organic phase.The aqueous phase, consisting of a divalent-lean lithium chloride-richstream, is removed for further processing and/or optional purification.The organic phase, consisting of the organic carrier solvent, theextraction compound and captured divalent ions can be treated with aconcentrated strong acid, for example HCl or H₂SO₄, such as a 20-36% HClsolution, to release the captured divalent ions. Optionally, thedivalent metal stream which includes released divalent ions present as,for example, metal chlorides, can be further purified. In certainembodiments, ion exchange, or other means, can be used to remove boronfrom the divalent metal stream. Both the divalent metal stream and thedivalent-lean lithium chloride-rich stream can be concentrated asdesired, by means described herein. For example, the divalent-leanlithium chloride-rich stream can be concentrated by evaporation orsolvent extraction.

The liquid extraction process is highly pH dependent, and the pH ismaintained such that divalent ions are removed from solution whilelithium ions remain. For example, in embodiments using Cyanex® 272, itis desirable to keep the pH at less than about 5.25, alternatively lessthan about 5, alternatively less than about 4.8, alternatively less thanabout 4.6, and alternatively less than about 4.5. At a pH of about 4.5,at least about 70% of calcium is removed from solution, at least about80 of magnesium is removed from solution, and at least about 99% ofmanganese is removed, while less than 2% of lithium is removed. Thus, atthe lower pH, the Cyanex® 272 shows very good selectivity for theextraction of calcium, magnesium and manganese over lithium.

The liquid extraction process can be performed over a wide variety oftemperatures, preferably between about 50° C. and 100° C., alternativelybetween about 60° C. and 80° C.; alternatively between about 70° C. and90° C.

The ratio of the organic extraction solution (which includes theextraction compound and carrier solvent) to the lithium-rich stream canbe between about 1:4 and 4:1, alternatively between about 1:4 and 1:1,alternatively between about 1:2 and 2:1; alternatively between about 1:1and 4:1.

In certain embodiments, the process for the extraction of one or moredivalent ion, such as calcium, magnesium, manganese, and/or zinc caninclude more than one column for the extraction thereof. For example, incertain embodiments, two columns can be employed in series to increasethe amount of divalent ions that are removed.

After removal of the one or more divalent ions, the ions can berecovered and separated, by known means, and supplied to an alternateprocess.

In certain embodiments, the process may include means for theneutralization of any lithium carbonate that is included in the sodiumchloride solution, such as by neutralizing the solution by adding aneffective amount of hydrochloric acid or like acid. In embodimentswherein the lithium carbonate can be effectively removed, the solutioncan be recycled to the electrochemical cell, however, any lithiumcarbonate included therein may cause problems with the performance ofthe electrochemical cell.

It is understood that certain processes and procedures described hereincan be performed in whole or in part. For example, it is understood thatthe process for the concentration of the lithium chloride containingstream by solvent extraction can be practiced with all or none of theother process steps that are described herein.

As used herein, the terms silica and silicates may be usedinterchangeably as it is understood that both terms are used to describesilicon based precipitates that are generated from geothermal brinesolutions.

EXAMPLES Example 1. Carbonation of Sodium Hydroxide

Carbonation of sodium hydroxide was carried out using a 3 liter jacketedreactor with a heating system (manufactured by Syrris Reactor Systems,UK). The reaction was carried out at a temperature of about 95° C. usinga one liter of a 9.5 M solution of sodium hydroxide ( 27.5% solids).Carbon dioxide was supplied for about 1 hour at the rate of 3 L/min.(totaling approximately 8 moles, approximately 1.7 molar equivalents) toensure the complete conversion of sodium hydroxide. At the end of thecarbonation of the sodium hydroxide solution, a clear solution of sodiumcarbonate was obtained, at which point the carbonation reaction wasstopped and heating of the sodium carbonate solution was continued forfew minutes. To the clear solution, lithium carbonate seeds were addedbefore reacting it with a lithium chloride solution (404 g lithiumchloride in 1000 mL). Experimental yield was 95%. Yields varied forother similar reactions depending upon experimental conditions and wereas high as about 100% in some cases. The purity of the isolated lithiumcarbonate was approximately 96.6% before washing.

Before the first washing of the product stream, the lithium carbonatehad the following impurities: Na (71 mg/kg), Ca (2.8 mg/kg), Mg (2.1mg/kg), Fe (0.3 mg/kg), Ba (0.1 mg/kg), Mn (0.08 mg/kg), and Sr (0.03mg/kg), for a purity of about 78.4%. After washing with approximately2-3 volume equivalents of water, the sodium concentration is reduced toundetectable levels and the lithium carbonate had the followingimpurities: Mg (5.9 mg/kg), Ca (2.9 mg/kg), Ba (0.4 mg/kg), Fe (0.4mg/kg), Mn (0.07 mg/kg), and Sr (0.07 mg/kg), for a purity of greaterthan 99%.

The washing conditions may affect the amount of sodiumcarbonate/chloride entrained in the lithium carbonate product.

Example 2

The electrolysis process converts a purified, concentrated lithiumchloride solution into a concentrated lithium hydroxide solution forsubsequent conversion to lithium bicarbonate. The limiting factordetermining the efficiency of the electrochemical cell is theconcentration of lithium hydroxide in the catholyte, due toback-migration of hydroxide across the membrane. Therefore, theexperiment was designed wherein the electrochemical cell was operated atfour different hydroxide concentrations to map the effect of the lithiumhydroxide concentration and determine the maximum concentration thatcould be prepared. The experiment was designed to measure the currentefficiency and energy utilization of the dialysis process as a functionof hydroxide concentration. Within the electrochemical cell, under anapplied field, lithium cations migrate from the anolyte to catholyte,while water present is electrolyzed to H₂ and OH⁻ at the cathode. Intheory, each electron passed in the external circuit corresponds to anincrease of one lithium hydroxide molecule in the catholyte, leading toan increase in concentration of lithium hydroxide with time. The maininefficiency in the process, the back migration of OH⁻ ions fromcatholyte to anolyte, is dependent on the OH⁻ concentration of thecatholyte. Therefore, the experiments reported here were performed withthe intention of maintaining the OH⁻ concentration of the catholyteconstant by adding water at a known rate. The efficiency of the reactionwas measured by comparing the actual rate of addition of water with thetheoretical addition.

Example 3. Electrolytic Production of Lithium Hydroxide from LithiumChloride

Experimental Set-Up. The electrolysis system consisted of theelectrolysis cell having anolyte and catholyte flow systems.Electrolysis of lithium chloride solutions was carried out using an FM01electrolyzer (a scale model of the FM21 electrolyzer used commerciallyin the chlor-alkali industry) manufactured by ICI. The electrolyzerincluded lantern blade-style electrodes (anode: ruthenium oxide coatedtitanium; and cathode: nickel), and a Nafion® 982 membrane. The activesurface area of each electrode was about 64 cm² (4×16 cm), and the cellgap (distance measured anode to cathode) was between about 12-13 mm. TheFM01 electrolyzer was operated with the flow parallel to the 16 cmdirection (as compared with a flow direction parallel to the 4 cmdimension, as it is intended to be operated), as this improved themanagement of chlorine and hydrogen gasses evolved from the electrodes.In addition, although anolyte and catholyte flows are normally fed fromopposite sides of the cell, in the present experiment, the anolyte andcatholyte were fed from the same side of the electrochemical cell.

The anolyte flow system included a feed tank, pump, degassing tank,chlorine scrubber, and collection tank. A lithium chloride solutionhaving a concentration of about 21% by weight was placed in the anolytefeed tank and heated to about 90° C. The heated solution was pumped intothe anode chamber of the cell in a single pass mode at a flow rate ofabout 20 cm³/min, corresponding to a face velocity of about 0.13 cm/s.Upon exiting the cell, the lithium chloride solution and entrainedchlorine gas (produced at the anode) were passed through into adegassing tank, which was equipped with a chlorine scrubber, to removethe chlorine. The lithium chloride solution was then pumped into acollection tank for storage.

The catholyte flow system included a feed tank, pump, and water feedsystem. Lithium hydroxide was placed in the feed tank and heated toabout 95° C. and fed to the cathode chamber of the electrochemical cellin recirculating mode at a flow rate of about 50 mL/min, correspondingto a face velocity of about 0.33 cm/s. Water was added continuously tothe system using a peristaltic pump to maintain a constant lithiumhydroxide concentration. The rate of addition was monitored by theweight loss of the water tank. Nitrogen was bubbled through thecatholyte recirculation tank to minimize the reaction of lithiumhydroxide and carbon dioxide from the air.

Table 1 summarizes the experimental conditions used in tests todetermine the effect of the concentration of the catholyte.

TABLE 1 Experimental parameters for electrolysis experiments. ParameterValue Current Density 3000 A/m⁻² Electrode Area 64 cm² Anolyte Volume 60cm³ Catholyte Volume 60 cm³ LiCl Inlet Concentration 21 wt % LiCl InletpH 0.5-0.7 Temperature 90° C. Time of Operation 2-3 hours Anolyte (LiCl)Flow Velocity 0.13 cm/s Catholyte (LiOH) Flow Velocity 0.33 cm/s

During operation of the electrochemical cell, samples were collected atthe catholyte inlet and outlet and anolyte outlet ports every 30minutes. Cell voltage was monitored at the cell terminals using ahandheld multimeter. The difference between the inlet and outletcatholyte hydroxide concentrations and the cell voltage were used tocalculate the efficiency and energy consumption of the cell.

Results

The results of the concentration of the catholyte are summarized inTable 2 and are shown in FIGS. 6 to 9. FIG. 6 demonstrates thedifficulty in maintaining a constant lithium hydroxide concentrationbased solely by adjusting the rate of water addition, in the absence ofreal-time measurements of the hydroxide concentration, because water canbe consumed or added to the catholyte by a variety of mechanisms,including electrolysis, evaporation, and migration across the membranewith lithium cations. In general, the data suggest that the higher theinitial concentration of lithium hydroxide, the more difficult the taskof maintaining the concentration constant through water addition.

The cell voltage was maintained at approximately 4.3-4.4 V for all ofthe experimental runs. FIG. 7 shows that cell voltage is relativelyindependent of hydroxide concentration, and implies that energyconsumption is largely driven by the electrical efficiency of theelectrode and membrane reactions. The cell gap in the FM01 electrolyzerused in this experiment (12-13 mm) is large compared to the cell gaptypically employed in commercial cells (2-3 mm), so a commercial cellwould be expected to have a lower cell voltage than those measured here.

FIG. 8 shows that current efficiency decreases with increasing lithiumhydroxide concentration. Without wishing to be bound by any one theory,it is believed this decrease in current efficiency may be due toincreased back-migration of hydroxide anions across the membrane fromthe catholyte to anolyte as the lithium hydroxide concentrationincreases. As shown in FIG. 9, this also results in increased energyconsumption, because all experiments were performed at the same currentdensity and the cell voltage was essentially constant. The experimentssuggest that a preferred concentration of lithium hydroxide in theelectrochemical cell may be between about 1-2 molar.

Table 2 summarizes the test results. As shown, lithium hydroxideproduction efficiency increases as lithium hydroxide concentrationdecreases, having an efficiency of up to about 80-88% for lithiumhydroxide solutions having a concentration of about 1 molar (2.4% byweight). Cell voltage is relatively independent of lithium hydroxideconcentration, so the efficiency also drives the energy requirement,which decreases to about 5 kWh/kg lithium hydroxide produced at aconcentration of about 1 molar. Lithium hydroxide production rate isgreatest with lower initial concentrations of lithium hydroxide.

TABLE 2 Summary of Results. LiOH LiOH Cell Production Energy conc. conc.Vol- Water Effi- Rate* kWh/ (Start) (Final) tage Added ciency kg LiOH/kg Test M M V g/min % m²/hr LiOH 1 2.57 3.28 4.37 0.5 35 0.94 15 2 1.621.88 4.45 5 65 1.74 8 3 0.94 0.92 4.28 11 80 2.14 5 4 0.69 0.89 4.33 1088 2.36 5.3 *Calculated (Production rate = 2.68 kg LiOH/m²/hr ×efficiency).

Example 4. Carbonation

Chemical Reactor. Lithium hydroxide was carbonated using a 3 L Syrrisautomated batch reactor system (Syrris Ltd. 27 Jarman Way, UK), havingcontrols for sensing pH, temperature, reagent addition, and sampleextraction. The electrolytic studies detailed above suggest thatElectrolysis of lithium chloride could at most generate 1 molar or 2.4wt % lithium hydroxide solution. Indeed, this concentration has beenfound to be ideal for conducting carbonation studies without cloggingissues under our experimental conditions.

Carbonation Reaction Kinetics. The carbonation reaction kinetics oflithium hydroxide were determined by monitoring pH and metal ionconcentration in solution (using Atomic Absorption) as the reactionprogressed. Approximately 84 g of lithium hydroxide monohydrate wasdissolved in 2000 mL of water to prepare a solution having aconcentration of about 1 molar (about 2.4% by weight). The reactorjacket was heated using a 30:70 water-glycol mixture and the temperatureof the lithium hydroxide solution was maintained at about 95° C. Thesolution was stirred at 250 RPM with a mechanical stirrer constantlyduring the carbonation. The carbonating gas tube was maintained at adepth of at least 6 cm in the caustic solution to begin with and the gasflow rate was continuously monitored using a flow meter (MathesonTri-Gas, USA). As the carbonation progressed, the pH of the solutionincreased slightly and the completion of the reaction was determined bysudden drop in the pH of the solution, soon after the carbon dioxideflow to the reactor was stopped. The drop in pH coincides with theformation of lithium bicarbonate, which is unstable at highertemperatures. Therefore, the solution was heating/stirring of thesolution was continued to decompose lithium bicarbonate that had formedinto lithium carbonate. The decomposition of the lithium bicarbonateresults in increased pH which stabilized over time. Lithium ionconcentration was monitored during the reaction and showed that excesscarbonation of the solution can lead to bicarbonate formation.

During carbonation, a slight molar excess of carbon dioxide was added tothe lithium hydroxide solution to account for poor mixing of the carbondioxide into the lithium hydroxide solution. After completion of thecarbonation reaction, the solution was hot filtered because the lithiumcarbonate solubility in water decreases at increased temperatures. Thefiltered solids were first dried at about 60° C. for about 18 hours, andwere then dried at about 120° C. for about 24 hrs to ensure theconversion of any residual lithium bicarbonate that may present in thesolids back to lithium carbonate. The carbonation reaction was repeatedseveral times with a 1 molar lithium hydroxide solution under slightlydifferent experimental conditions, and both with and without lithiumcarbonate seeds. The results are shown in Table 3. Seeding of lithiumhydroxide solution with lithium carbonate crystals improved yields. Athigher carbon dioxide flow rates (e.g., at 3 L/min and greater), theyield of the carbonation reaction remained high. As shown in Table 3,carbon dioxide feed was maintained at about 2 L/min, although the totalamount of carbon dioxide added varied between about 1.25 and 2.5 moles(i.e., between about 0.625 and 1.25 molar equivalents). Experiment 1 inTable 3 included the addition of nitrogen gas to the carbonation vessel.Experiments 3-5 in Table 3 included the addition of between about 0.6%and 1.2% by weight lithium hydroxide seeds. The results show thatincreased reaction rate can allow for a reduction in the reactor size,and reduced overall cost associated therewith.

TABLE 3 Carbonation Reaction of a 2.4% by Weight Solution of LiOH^(†)Overall Lithium Carbonation Carbonate Solids Exp. Reaction ConditionsYield (%)^(#) Recovered (%) 1 CO₂ (2LPM, 2.5 moles) + 100.0%    57%* N₂(3.7 LPM) 2 CO₂ (2LPM, 1.9 moles) 93% 73% 3 CO₂ (2LPM, 1.5 moles) + 99%82% 1.2% Li₂CO₃ seeds 4 CO₂ (2LPM, 1.25 moles) + 93% 78% 0.6% Li₂CO₃seeds 5 CO₂ (3LPM, 1.3 moles) + 96% 82% 1.2% Li₂CO₃ seeds ^(†)Preparedby mixing 84 g lithium hydroxide (LiOH•H₂0) in 2 L water. ^(#)Overallyield includes the amount of lithium carbonate/bicarbonate dissolved insolution and deposited inside the reactor walls. *excessively carbonatedand filtered without converting LiHCO₃ back into Li₂CO₃.

Example 5. Removal of Calcium, Manganese, and Magnesium

An extraction solution that includes 30% Cyanex 272 in Isopar M wasprepared. An aqueous lithium containing solution (having a compositionthat included: 3390 mg/L Li; 1740 mg/L Ca; 5.53 mg/L Mg; 142.5 mg/L Mn;1.45 mg/L Zn; 9.11 mg/L Ba; and 11.65 mg/L Sr) was contacted with theextraction solution in a ratio ranging from between 1:4 to 4:1 forapproximately 5 minutes in a jacketed solvent extraction vessel equippedwith an overhead stirrer at about 75° C. The pH of the solution in theextraction vessel was maintained at equilibrium at about 4.5 through theaddition of a sodium hydroxide solution. After mixing the extractionsolution and the aqueous lithium containing solution is complete, thesolution is allowed to stand and the organic and aqueous phases areseparated. Analysis of the resulting organic phase by ICP provided theamount of ions extracted from the aqueous solution and captured by theextraction compound, for the various reaction mixture are provided inTable 4, below. As shown, at the given pH and temperature, selectivityfor lithium is very low (i.e., less than 8%). At ratios of theextraction solution (identified in Table 4 as the organic solution) toaqueous lithium containing solution (identified as the aqueous solution)of 2:1 and greater, selectivity for calcium is greater than about 90%,selectivity for magnesium is greater than about 80% selectivity formanganese is about 100%, and selectivity for zinc is about 50%.

TABLE 4 Ratio of organic/ aqueous solutions 1:4 1:2 1:1 2:1 3:1 4:1 Li —8 — 0 6 8 Ca 32 60 79 92 95 96 Mg 70 82 86 87 84 81 Mn 99 100 100 100 9999 Zn 50 49 47 49 49 46 Ba 3 — — 13 21 25 Sr 1 — 4 26 39 47

Example 6. Extraction of Calcium, Manganese, and Magnesium

In another example, an extraction solution that includes 30% Cyanex 272in Linpar 1416-V was prepared. An aqueous lithium containing solution(having a composition that included: 3450 mg/L Li; and 1720 mg/L Ca) wascontacted with the extraction solution in a ratio ranging from between1:4 to 4:1 for approximately 5 minutes in a jacketed solvent extractionvessel equipped with an overhead stirrer at about 90° C. The pH of thesolution in the extraction vessel was maintained at equilibrium at about4.5 through the addition of a sodium hydroxide solution. After mixingthe extraction solution and the aqueous lithium containing solution iscomplete, the solution is allowed to stand and the organic and aqueousphases are separated. Analysis of the resulting organic phase by ICPprovided the amount of ions extracted from the aqueous solution andcaptured by the extraction compound. As shown in Table 5, at the givenpH and temperature, selectivity for lithium is very low (i.e., less than8%). As shown in the Table, lithium extraction is minimized at ratios ofthe extraction solution (identified in Table 4 as the organic solution)to aqueous lithium containing solution (identified as the aqueoussolution) of 2:1 and lower. At increased ratios, both calcium extractionand lithium extraction increase. Magnesium extraction is at least about81%, regardless of the ratio of organic to aqueous solution, andmanganese extraction is similarly about 100% for all ratios of organicto aqueous solution.

TABLE 5 Ratio of organic/ aqueous solutions 1:4 1:2 1:1 2:1 3:1 4:1 Li —— 1 2 11 20 Ca 29 48 63 82 93 96 Mg 81 86 87 88 89 85 Mn 100 100 10 99100 99 Zn 53 52 53 52 56 56 Ba — — — 4 18 33 Sr — 0 2 13 33 54

The methods described herein are suitable for the recovery of lithiumfrom brines or solutions having low or high lithium concentrations, inaddition to brines or solutions that include significant concentrationsof other ions, including multivalent ions.

As is understood in the art, not all equipment or apparatuses are shownin the figures. For example, one of skill in the art would recognizethat various holding tanks and/or pumps may be employed in the presentmethod.

The singular forms “a”, “an” and “the” include plural referents, unlessthe context clearly dictates otherwise.

Optional or optionally means that the subsequently described event orcircumstances may or may not occur. The description includes instanceswhere the event or circumstance occurs and instances where it does notoccur.

Ranges may be expressed herein as from about one particular value,and/or to about another particular value. When such a range isexpressed, it is to be understood that another embodiment is from theone particular value and/or to the other particular value, along withall combinations within said range.

Throughout this application, where patents or publications arereferenced, the disclosures of these references in their entireties areintended to be incorporated by reference into this application, in orderto more fully describe the state of the art to which the inventionpertains, except when these reference contradict the statements madeherein.

As used herein, recitation of the term about and approximately withrespect to a range of values should be interpreted to include both theupper and lower end of the recited range.

Although the present invention has been described in detail, it shouldbe understood that various changes, substitutions, and alterations canbe made hereupon without departing from the principle and scope of theinvention. Accordingly, the scope of the present invention should bedetermined by the following claims and their appropriate legalequivalents.

1-20. (canceled)
 21. A process for recovery of lithium from a geothermalbrine, the process comprising the steps of: removing impurities from ageothermal brine; recovering lithium chloride from the geothermal brineto produce a lithium chloride-rich stream; concentrating the lithiumchloride in the lithium chloride-rich stream using reverse osmosis; andconverting the lithium chloride in the lithium chloride-rich stream tolithium carbonate, lithium hydroxide, or both.
 22. The process of claim21, wherein the geothermal brine is a Salton Sea geothermal brine. 23.The process of claim 21, wherein removing impurities from the geothermalbrine comprises removing iron and silica from the geothermal brine usingoxidation and co-precipitation.
 24. The process of claim 21, wherein thelithium chloride is further concentrated via thermal or otherconcentration methods to produce a lithium chloride-rich stream.
 25. Theprocess of claim 24, wherein a concentration of lithium chloride in thelithium chloride-rich stream is between 1 wt. % and 42 wt. %.
 26. Theprocess of claim 21, wherein converting the lithium chloride furthercomprises the steps of: converting the lithium chloride in the lithiumchloride-rich stream to lithium carbonate using a crystallizer; and/orconcentrating the lithium chloride in the lithium chloride-rich streamusing a solvent extraction process, and converting the lithium chloridein the lithium chloride-rich stream to lithium hydroxide usingelectrolysis.
 27. The process of claim 26, further comprising the stepsof: recovering the lithium carbonate from the crystallizer; andconverting the lithium carbonate to lithium hydroxide.
 28. The processof claim 26, further comprising removing calcium, magnesium and/or boronfrom the lithium chloride-rich stream to form a substantially calcium,magnesium and/or boron free brine.
 29. The process of claim 26, furthercomprising removing calcium and magnesium from the lithium chloride-richstream using precipitation to form a substantially calcium and magnesiumfree brine.
 30. The process of claim 26, further comprising removingboron from the lithium chloride-rich stream using an ion exchange and/orsolvent extraction to form a substantially calcium, magnesium and/orboron free brine.
 31. The process of claim 26, further comprisingremoving any remaining divalent ions from the lithium chloride-richstream using ion exchange.
 32. A process for recovery of lithium from ageothermal brine, the process comprising the steps of: removingimpurities from a geothermal brine; recovering lithium chloride from thegeothermal brine to produce a lithium chloride-rich stream; andconcentrating the lithium chloride in the lithium chloride-rich streamusing reverse osmosis.
 33. The process of claim 32, wherein thegeothermal brine is a Salton Sea geothermal brine.
 34. The process ofclaim 32, wherein removing impurities from the geothermal brinecomprises removing iron and silica from the geothermal brine usingoxidation and co-precipitation.
 35. The process of claim 32, wherein thelithium chloride is further concentrated via thermal or otherconcentration methods to produce a lithium chloride-rich stream.
 36. Theprocess of claim 35, wherein a concentration of lithium chloride in thelithium chloride-rich stream is between 1 wt. % and 42 wt. %.
 37. Theprocess of claim 32, further comprising removing calcium, magnesiumand/or boron from the lithium chloride-rich stream to form asubstantially calcium, magnesium and/or boron free brine.
 38. Theprocess of claim 32, further comprising removing calcium and magnesiumfrom the lithium chloride-rich stream using precipitation to form asubstantially calcium and magnesium free brine.
 39. The process of claim32, further comprising removing boron from the lithium chloride-richstream using an ion exchange and/or solvent extraction to form asubstantially calcium, magnesium and/or boron free brine.
 40. Theprocess of claim 32, further comprising removing any remaining divalentions from the lithium chloride-rich stream using ion exchange.